PHYSICAL SETTING CHEMISTRY - JMAP · 2017-01-01 · Part A Answer all questions in this part. Directions (1–30): For each statement or question, record on your separate answer sheet

The University of the State of New York

REGENTS HIGH SCHOOL EXAMINATION

PHYSICAL SETTING

CHEMISTRYWednesday, August 17, 2016 — 8:30 to 11:30 a.m., only

This is a test of your knowledge of chemistry. Use that knowledge to answer allquestions in this examination. Some questions may require the use of the 2011 EditionReference Tables for Physical Setting/Chemistry. You are to answer all questions in allparts of this examination according to the directions provided in this examinationbooklet.

A separate answer sheet for Part A and Part B–1 has been provided to you. Followthe instructions from the proctor for completing the student information on youranswer sheet. Record your answers to the Part A and Part B–1 multiple-choicequestions on this separate answer sheet. Record your answers for the questions inPart B–2 and Part C in your separate answer booklet. Be sure to fill in the heading onthe front of your answer booklet.

All answers in your answer booklet should be written in pen, except for graphs anddrawings, which should be done in pencil. You may use scrap paper to work out theanswers to the questions, but be sure to record all your answers on your separateanswer sheet or in your answer booklet as directed.

When you have completed the examination, you must sign the statement printedon your separate answer sheet, indicating that you had no unlawful knowledge of thequestions or answers prior to the examination and that you have neither given norreceived assistance in answering any of the questions during the examination. Youranswer sheet and answer booklet cannot be accepted if you fail to sign thisdeclaration.

DO NOT OPEN THIS EXAMINATION BOOKLET UNTIL THE SIGNAL IS GIVEN.

The possession or use of any communications device is strictly prohibited when taking this examination. If you have or use any communications device, no matter howbriefly, your examination will be invalidated and no score will be calculated for you.

Notice. . .

A four-function or scientific calculator and a copy of the 2011 Edition Reference Tables forPhysical Setting/Chemistry must be available for you to use while taking this examination.

P.S./CHEMISTRYP.S./CHEMISTRY

Part A

Answer all questions in this part.

Directions (1–30): For each statement or question, record on your separate answer sheet the number of theword or expression that, of those given, best completes the statement or answers the question. Some questionsmay require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.

P.S./Chem.–Aug. ’16 [2]

1 Which change occurs when an atom in an excitedstate returns to the ground state?(1) Energy is emitted.(2) Energy is absorbed.(3) The number of electrons decreases.(4) The number of electrons increases.

2 The valence electrons in an atom of phosphorusin the ground state are all found in(1) the first shell (3) the third shell(2) the second shell (4) the fourth shell

3 Which two elements have the most similarchemical properties?(1) beryllium and magnesium(2) hydrogen and helium(3) phosphorus and sulfur(4) potassium and strontium

4 Which phrase describes a compound that consists of two elements?(1) a mixture in which the elements are in a

variable proportion(2) a mixture in which the elements are in a

fixed proportion(3) a substance in which the elements are

chemically combined in a variable proportion(4) a substance in which the elements are

chemically combined in a fixed proportion

5 The formula mass of a compound is the(1) sum of the atomic masses of its atoms(2) sum of the atomic numbers of its atoms(3) product of the atomic masses of its atoms(4) product of the atomic numbers of its atoms

6 The arrangement of the elements from left toright in Period 4 on the Periodic Table is based on(1) atomic mass(2) atomic number(3) the number of electron shells(4) the number of oxidation states

7 Which diatomic molecule is formed when thetwo atoms share six electrons?(1) H2 (3) O2(2) N2 (4) F2

8 Which formula represents a polar molecule?(1) O2 (3) NH3(2) CO2 (4) CH4

9 Which element is least likely to undergo achemical reaction?

(1) lithium (3) fluorine(2) carbon (4) neon

10 Which element has a melting point higher thanthe melting point of rhenium?(1) iridium (3) tantalum(2) osmium (4) tungsten

11 Which property can be defined as the ability ofa substance to be hammered into thin sheets?(1) conductivity (3) melting point(2) malleability (4) solubility

12 Which list of elements consists of a metal, ametalloid, and a noble gas?(1) aluminum, sulfur, argon(2) magnesium, sodium, sulfur(3) sodium, silicon, argon(4) silicon, phosphorus, chlorine

P.S./Chem.–Aug. ’16 [3] [OVER]

13 Which sample of matter has a crystal structure?(1) Hg(ℓ) (3) NaCl(s)(2) H2O(ℓ) (4) CH4(g)

14 One mole of liquid water and one mole of solidwater have different

(1) masses(2) properties(3) empirical formulas(4) gram-formula masses

15 Which substance can not be broken down by achemical change?(1) butanal (3) gold(2) propene (4) water

16 Which statement describes particles of an idealgas, based on the kinetic molecular theory?(1) Gas particles are separated by distances

smaller than the size of the gas particles.(2) Gas particles do not transfer energy to each

other when they collide.(3) Gas particles have no attractive forces

between them.(4) Gas particles move in predictable, circular

motion.

17 Which expression could represent the concentration of a solution?(1) 3.5 g (3) 3.5 mL(2) 3.5 M (4) 3.5 mol

18 Which form of energy is associated with the random motion of the particles in a sample ofwater?(1) chemical energy (3) nuclear energy(2) electrical energy (4) thermal energy

19 Which change is most likely to occur when amolecule of H2 and a molecule of I2 collide withproper orientation and sufficient energy?(1) a chemical change, because a compound is

formed(2) a chemical change, because an element is

formed(3) a physical change, because a compound is

formed(4) a physical change, because an element is

formed

20 Which changes can reach dynamic equilibrium?(1) nuclear changes, only(2) chemical changes, only(3) nuclear and physical changes(4) chemical and physical changes

21 What occurs when a reaction reaches equilibrium?(1) The concentration of the reactants increases.(2) The concentration of the products increases.(3) The rate of the forward reaction is equal to

the rate of the reverse reaction.(4) The rate of the forward reaction is slower

than the rate of the reverse reaction.

22 In terms of potential energy, PE, which expression defines the heat of reaction for achemical change?

(1)

(2)

(3)

(4)

23 Systems in nature tend to undergo changes thatresult in(1) lower energy and lower entropy(2) lower energy and higher entropy(3) higher energy and lower entropy(4) higher energy and higher entropy

24 What occurs when Cr3� ions are reduced toCr2� ions? (1) Electrons are lost and the oxidation number

of chromium increases.(2) Electrons are lost and the oxidation number

of chromium decreases.(3) Electrons are gained and the oxidation number

of chromium increases.(4) Electrons are gained and the oxidation number

of chromium decreases.

PEPE

reactants

products

PEPE

products

reactants

PE PE productsreactants −

PE PEproducts − reactants

P.S./Chem.–Aug. ’16 [4]

25 Where do reduction and oxidation occur in anelectrolytic cell?(1) Both occur at the anode.(2) Both occur at the cathode.(3) Reduction occurs at the anode, and oxidation

occurs at the cathode.(4) Reduction occurs at the cathode, and oxidation

occurs at the anode.

26 Which compound is an electrolyte?(1) H2O (3) H3PO4(2) C2H6 (4) CH3OH

27 When the hydronium ion concentration of anaqueous solution is increased by a factor of 10,the pH value of the solution(1) decreases by 1 (3) decreases by 10(2) increases by 1 (4) increases by 10

28 The stability of isotopes is related to the ratio ofwhich particles in the atoms?(1) electrons and protons(2) electrons and positrons(3) neutrons and protons(4) neutrons and positrons

29 Which radioisotope has the fastest rate ofdecay?(1) 14C (3) 53Fe(2) 37Ca (4) 42K

30 The atomic mass of an element is the weightedaverage of the atomic masses of(1) the least abundant isotopes of the element(2) the naturally occurring isotopes of the

element(3) the artificially produced isotopes of the

element(4) the natural and artificial isotopes of the

element


31 Which list of elements is arranged in order ofincreasing electronegativity?(1) Be, Mg, Ca (3) K, Ca, Sc(2) F, Cl, Br (4) Li, Na, K

32 The table below gives the masses of two differentsubatomic particles found in an atom.

Subatomic Particles and Their Masses

Which of the subatomic particles are each pairedwith their corresponding name?(1) X, proton and Z, electron(2) X, proton and Z, neutron(3) X, neutron and Z, proton(4) X, electron and Z, proton

33 Which electron configuration represents anexcited state for an atom of calcium?(1) 2-8-7-1 (3) 2-8-7-3(2) 2-8-7-2 (4) 2-8-8-2

34 At STP, graphite and diamond are two solidforms of carbon. Which statement explains whythese two forms of carbon differ in hardness?(1) Graphite and diamond have different ionic

radii.(2) Graphite and diamond have different

molecular structures.(3) Graphite is a metal, but diamond is a

nonmetal.(4) Graphite is a good conductor of electricity,

but diamond is a poor conductor of electricity.

35 Which equation shows conservation of charge?(1) Cu � Ag�

→ Cu2� � Ag(2) Mg � Zn2�

→ 2Mg2� � Zn

(3) 2F2 � Br� → 2F� � Br2

(4) 2I� � Cl2 → I2 � 2Cl�

36 What occurs when potassium reacts with chlorine to form potassium chloride?(1) Electrons are shared and the bonding is ionic.(2) Electrons are shared and the bonding is

covalent.(3) Electrons are transferred and the bonding is

ionic.(4) Electrons are transferred and the bonding is

covalent.

37 Given the balanced equation representing areaction:

H2 � energy → H � H

What occurs as bonds are broken in one mole ofH2 molecules during this reaction?(1) Energy is absorbed and one mole of

unbonded hydrogen atoms is produced.(2) Energy is absorbed and two moles of

unbonded hydrogen atoms are produced.(3) Energy is released and one mole of unbonded

hydrogen atoms is produced.(4) Energy is released and two moles of

unbonded hydrogen atoms are produced.

38 Which pair of atoms has the most polar bond?(1) H−Br (3) I−Br(2) H−Cl (4) I−Cl

Subatomic

Particle

Mass

(g)X 1.67 � 10�24

Z 9.11 � 10�28

Part B–1


Directions (31–50): For each statement or question, record on your separate answer sheet the number of theword or expression that, of those given, best completes the statement or answers the question. Some questionsmay require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.

P.S./Chem.–Aug. ’16 [6]

39 Which two notations represent isotopes of thesame element?(1) 14

7N and 187N (3) 14

7N and 1710Ne

(2) 207N and 20

10Ne (4) 197N and 16

10Ne

40 The graph below shows the volume and themass of four different substances at STP.

Which of the four substances has the lowestdensity?(1) A (3) C(2) B (4) D

41 What is the total amount of heat required tocompletely melt 347 grams of ice at its meltingpoint?(1) 334 J (3) 116 000 J(2) 1450 J (4) 784 000 J

42 As the temperature of a reaction increases, it isexpected that the reacting particles collide(1) more often and with greater force(2) more often and with less force(3) less often and with greater force(4) less often and with less force

43 Given the formula representing a compound:

What is an IUPAC name for this compound?(1) ethyl propanoate (3) 3-hexanone(2) propyl ethanoate (4) 4-hexanone

44 A voltaic cell converts chemical energy to(1) electrical energy with an external power

source(2) nuclear energy with an external power

source(3) electrical energy without an external power

source(4) nuclear energy without an external power

source

45 Which acid and base react to form water andsodium sulfate?(1) sulfuric acid and sodium hydroxide(2) sulfuric acid and potassium hydroxide(3) sulfurous acid and sodium hydroxide(4) sulfurous acid and potassium hydroxide

46 Given the equation representing a reaction:

H2CO3 � NH3 → NH4� � HCO3

�

According to one acid-base theory, the compound NH3 acts as a base because it(1) accepts a hydrogen ion(2) donates a hydrogen ion(3) accepts a hydroxide ion(4) donates a hydroxide ion

47 Which statement describes characteristics of a0.01 M KOH(aq) solution?(1) The solution is acidic with a pH less than 7.(2) The solution is acidic with a pH greater than 7.(3) The solution is basic with a pH less than 7.(4) The solution is basic with a pH greater than 7.

00

Volume

Mas

s

AB

C

D

H

H

C C

H

C

H

HH

C C C H

H H

HH

H

O


48 Four statements about the development of the atomic model are shown below.

A: Electrons have wavelike properties.B: Atoms have small, negatively charged particles.C: The center of an atom is a small, dense nucleus.D: Atoms are hard, indivisible spheres.

Which order of statements represents the historical development of the atomic model?(1) C → D → A → B(2) C → D → B → A(3) D → B → A → C(4) D → B → C → A

49 Five cubes of iron are tested in a laboratory. The tests and the results are shown in the table below.

Iron Tests and the Results

Which tests demonstrate chemical properties?(1) 1, 3, and 4 (3) 2 and 4(2) 1, 3, and 5 (4) 2 and 5

Test Procedure Result

1 A cube of Fe is hit with a hammer. The cube is flattened.

2 A cube of Fe is placed in 3 M HCl(aq). Bubbles of gas form.

3 A cube of Fe is heated to 1811 K. The cube melts.

4 A cube of Fe is left in damp air. The cube rusts.

5 A cube of Fe is placed in water. The cube sinks.

50 A rigid cylinder with a movable piston contains a sample of helium gas. The temperature of the gas is heldconstant as the piston is pulled outward. Which graph represents the relationship between the volume ofthe gas and the pressure of the gas?

Pre

ssu

reVolume

Pre

ssu

re

VolumeP

ress

ure

Volume

Pre

ssu

re

Volume

( 1 ) ( 3 )

( 2 ) ( 4 )

P.S./Chem.–Aug. ’16 [8]


51 What is the empirical formula for C6H12? [1]

52 Using Table G, determine the minimum mass of NaCl that must be dissolved in 200. grams of water to produce a saturated solution at 90.°C. [1]

53 State the physical property that makes it possible to separate a solution by distillation. [1]

Base your answers to questions 54 and 55 on the information below and on your knowledge of chemistry.

A beaker contains a liquid sample of a molecular substance. Both the beaker and theliquid are at 194 K. The graph below represents the relationship between temperature andtime as the beaker and its contents are cooled for 12 minutes in a refrigerated chamber.

54 State what happens to the average kinetic energy of the molecules in the sample duringthe first 3 minutes. [1]

55 Identify the physical change occurring during the time interval, minute 4 to minute 9. [1]

120.

100.

80.

140.

160.

180.

200.Cooling Curve for a Substance

Time (min)

Tem

per

atu

re (

K)

0 1 2 3 4 5 6 7 8 9 10 11 12

Part B–2


Directions (51–65): Record your answers in the spaces provided in your answer booklet. Some questionsmay require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.

P.S./Chem.–Aug. ’16 [10]

Base your answers to questions 56 through 59 on the information below and on your knowledge of chemistry.

The equation below represents a reaction between propene and hydrogen bromide.

Cyclopropane, an isomer of propene, has a boiling point of –33ºC at standard pressureand is represented by the formula below.

56 Explain why this reaction can be classified as a synthesis reaction. [1]

57 Identify the class of organic compounds to which the product of this reaction belongs. [1]

58 Explain, in terms of molecular formulas and structural formulas, why cyclopropane is anisomer of propene. [1]

59 Convert the boiling point of cyclopropane at standard pressure to kelvins. [1]

CH

C

H

CH

H

HH

H

H

C

H

C C

H

H

H

H Br H

H

C

H

H

C

Br

H

C

H

H



The radius of a lithium atom is 130. picometers, and the radius of a fluorine atomis 60. picometers. The radius of a lithium ion, Li�, is 59 picometers, and the radius of a fluoride ion, F�, is 133 picometers.

60 Compare the radius of a fluoride ion to the radius of a fluorine atom. [1]

61 Explain, in terms of subatomic particles, why the radius of a lithium ion is smaller thanthe radius of a lithium atom. [1]

62 In the space in your answer booklet, draw a Lewis electron-dot diagram for a fluoride ion. [1]

63 Describe the general trend in atomic radius as each element in Period 2 is consideredin order from left to right. [1]

Base your answers to questions 64 and 65 on the information below and on your knowledge of chemistry.

Nuclear fission reactions can produce different radioisotopes. One of these radioisotopesis Te-137, which has a half-life of 2.5 seconds. The diagram below represents one of the many nuclear fission reactions.

64 State evidence that this nuclear reaction represents transmutation. [1]

65 Complete the nuclear equation in your answer booklet for the beta decay of Zr-97, bywriting an isotopic notation for the missing product. [1]

13752Te

9740Zr

10n

23592U1

0n10n

+ energy


Stamping an identification number into the steel frame of a bicycle compresses thecrystal structure of the metal. If the number is filed off, there are scientific ways to revealthe number.

One method is to apply aqueous copper(II) chloride to the number area. The Cu2� ionsreact with some iron atoms in the steel frame, producing copper atoms that show the pattern of the number. The ionic equation below represents this reaction.

Fe(s) � Cu2�(aq) → Fe2�(aq) � Cu(s)

Another method is to apply hydrochloric acid to the number area. The acid reacts withthe iron, producing bubbles of hydrogen gas. The bubbles form faster where the metal wascompressed, so the number becomes visible. The equation below represents this reaction.

2HCl(aq) � Fe(s) → FeCl2(aq) � H2(g)

66 Explain why the Fe atoms in the bicycle frame react with the Cu2� ions. [1]

67 Determine the number of moles of hydrogen gas produced when 0.001 mole ofHCl(aq) reacts completely with the iron metal. [1]

68 Write a balanced half-reaction equation for the reduction of the hydrogen ions to hydrogen gas. [1]

69 Describe one change in the HCl(aq) that will increase the rate at which hydrogen bubbles are produced when the acid is applied to the steel frame. [1]

P.S./Chem.–Aug. ’16 [12]

Part C


Directions (66–85): Record your answers in the spaces provided in your answer booklet. Some questionsmay require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.



In an investigation, aqueous solutions are prepared by completely dissolving a differentamount of NaCl(s) in each of four beakers containing 100.00 grams of H2O(ℓ) at room temperature. Each solution is heated and the temperature at which boiling occurred ismeasured. The data are recorded in the table below.

Boiling Point Data for Four NaCl(aq) Solutions

70 Identify the solute and the solvent used in this investigation. [1]

71 Show a numerical setup for calculating the percent by mass of NaCl in the solution in beaker 4. [1]

72 Explain, in terms of ions, why the ability to conduct an electric current is greater for thesolution in beaker 4 than for the solution in beaker 1. [1]

73 State the relationship between the concentration of ions and the boiling point for thesesolutions. [1]

Beaker

Number

Mass of H2O(ℓ)(g)

Mass of NaCl(s)

Dissolved

(g)

Boiling Point of

Solution

(°C)

1 100.00 8.76 101.5

2 100.00 17.52 103.1

3 100.00 26.28 104.6

4 100.00 35.04 106.1


One type of voltaic cell, called a mercury battery, uses zinc and mercury(II) oxide togenerate an electric current. Mercury batteries were used because of their miniature size,even though mercury is toxic. The overall reaction for a mercury battery is given in theequation below.

Zn(s) � HgO(s) → ZnO(s) + Hg(ℓ)

74 Determine the change in the oxidation number of zinc during the operation of the cell. [1]

75 Compare the number of moles of electrons lost to the number of moles of electronsgained during the reaction. [1]

76 Using information in the passage, state one risk and one benefit of using a mercury battery. [1]


A company produces a colorless vinegar that is 5.0% HC2H3O2 in water. Using thymolblue as an indicator, a student titrates a 15.0-milliliter sample of the vinegar with 43.1 milliliters of a 0.30 M NaOH(aq) solution until the acid is neutralized.

77 Based on Table M, what is the color of the indicator in the vinegar solution before anybase is added? [1]

78 Identify the negative ion in the NaOH(aq) used in this titration. [1]

79 The concentration of the base used in this titration is expressed to what number of significant figures? [1]

80 Determine the molarity of the HC2H3O2 in the vinegar sample, using the titration data. [1]

P.S./Chem.–Aug. ’16 [14]


In industry, ethanol is primarily produced by two different reactions. One processinvolves the reaction of glucose in the presence of an enzyme that acts as a catalyst. Theequation below represents this reaction.

Equation 1: C6H12O6 enzyme 2CH3CH2OH � 2CO2

glucose ethanol

In another reaction, ethanol is produced from ethene and water. The equation belowrepresents this reaction in which H2SO4 is a catalyst.

Equation 2: CH2CH2 + H2OH2SO4 CH3CH2OH

Industrial ethanol can be oxidized using a catalyst to produce ethanal. The equation representing this oxidation is shown below.

Equation 3: CH3CH2OH catalyst CH3CHO � H2

81 Identify the element that causes the reactant in equation 1 to be classified as an organiccompound. [1]

82 Identify the type of organic reaction represented by equation 1. [1]

83 Explain why the hydrocarbon in equation 2 is unsaturated. [1]

84 Explain, in terms of intermolecular forces, why ethanol has a much higher boiling pointthan ethene, at standard pressure. [1]

85 Draw a structural formula for the organic product in equation 3. [1]

P.S./Chem.–Aug. ’16 [15]


Printed on Recycled Paper

The University of the State of New York


PHYSICAL SETTINGCHEMISTRY

Wednesday, August 17, 2016 — 8:30 to 11:30 a.m., only

ANSWER BOOKLET

Student . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Sex: � Female

Teacher . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

School . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Grade . . . . . . . . .

Record your answers for Part B–2 and Part C in this booklet.

� Male

51

52 g

53

54

55

Part B–2

P.S./Chem. Answer Booklet–Aug. ’16 [2]

56

57

58

59 K

60

61

P.S./Chem. Answer Booklet–Aug. ’16 [3] [OVER]

62

63

64

65 9740 Zr → e � _________0

1�


66

67 mol

68

69

70 Solute:

Solvent:

71

72

Part C

P.S./Chem. Answer Booklet–Aug. ’16 [5] [OVER]

73

74 From _________ to _________

75

76 Risk:

Benefit:

77

78

79

80 M


81

82

83

84

85


Printed on Recycled Paper

FOR TEACHERS ONLYThe University of the State of New York


PHYSICAL SETTING/CHEMISTRY

Wednesday, August 17, 2016 — 8:30 to 11:30 a.m., only

SCORING KEY AND RATING GUIDE

P.S.–CH

Directions to the Teacher:Refer to the directions on page 2 before rating student papers.

Updated information regarding the rating of this examination may be posted on the New YorkState Education Department’s web site during the rating period. Check this web site at:http://www.p12.nysed.gov/assessment/ and select the link “Scoring Information” for any recentlyposted information regarding this examination. This site should be checked before the rating processfor this examination begins and several times throughout the Regents Examination period.

Part A and Part B–1

Allow 1 credit for each correct response.

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Part A

Part B–1

P.S./Chem. Rating Guide–Aug. ’16 [2]

Directions to the Teacher

Follow the procedures below for scoring student answer papers for the Regents Examination inPhysical Setting/Chemistry. Additional information about scoring is provided in the publication InformationBooklet for Scoring Regents Examinations in the Sciences.

Do not attempt to correct the student’s work by making insertions or changes of any kind.If the student’s responses for the multiple-choice questions are being hand scored prior to beingscanned, the scorer must be careful not to make any marks on the answer sheet except to recordthe scores in the designated score boxes. Marks elsewhere on the answer sheet will interferewith the accuracy of the scanning.

Allow 1 credit for each correct response.

At least two science teachers must participate in the scoring of the Part B–2 and Part C open-endedquestions on a student’s paper. Each of these teachers should be responsible for scoring a selected numberof the open-ended questions on each answer paper. No one teacher is to score more than approximatelyone-half of the open-ended questions on a student’s answer paper. Teachers may not score their own students’ answer papers.

Students’ responses must be scored strictly according to the Scoring Key and Rating Guide. For open-ended questions, credit may be allowed for responses other than those given in the rating guide if theresponse is a scientifically accurate answer to the question and demonstrates adequate knowledge, as indicated by the examples in the rating guide. On the student’s separate answer sheet, for each question,record the number of credits earned and the teacher’s assigned rater/scorer letter.

Fractional credit is not allowed. Only whole-number credit may be given for a response. If the studentgives more than one answer to a question, only the first answer should be rated. Units need not be givenwhen the wording of the questions allows such omissions.

For hand scoring, raters should enter the scores earned in the appropriate boxes printed on the separate answer sheet. Next, the rater should add these scores and enter the total in the box labeled “Total Raw Score.” Then the student’s raw score should be converted to a scale score by using the conversion chart that will be posted on the Department’s web site at: http://www.p12.nysed.gov/assessment/on Wednesday, August 17, 2016. The student’s scale score should be entered in the box labeled “Scale Score” on the student’s answer sheet. The scale score is the student’s final examination score.

Schools are not permitted to rescore any of the open-ended questions on this exam after eachquestion has been rated once, regardless of the final exam score. Schools are required to ensurethat the raw scores have been added correctly and that the resulting scale score has been determined accurately.

Because scale scores corresponding to raw scores in the conversion chart may change from one administration to another, it is crucial that, for each administration, the conversion chart provided for thatadministration be used to determine the student’s final score.


Part B–2

Allow a total of 15 credits for this part. The student must answer all questions in this part.

51 [1] Allow 1 credit for CH2. The order of the elements can vary.

52 [1] Allow 1 credit for any value from 78 g to 82 g inclusive.

53 [1] Allow 1 credit. Acceptable responses include, but are not limited to:

boiling point

boiling temperature


The average kinetic energy decreases.

The average KE goes down.


freezing

solidification

liquid to solid


Two substances react to produce one substance.

This product is formed by chemically combining two substances.

Two molecules produce a more complex molecule.

One compound is formed from two compounds.


halide

halocarbon

alkyl halide

halogenalkane



The molecular formulas for the two compounds are the same, but the structural formulas aredifferent.

Both molecules have the same number of C atoms and the same number of H atoms, but havea different arrangement of atoms.

Both compounds are C3H6, but have different structures.

Both compounds are C3H6, but one has a ring and one has a double bond.

59 [1] Allow 1 credit for 240. K. Significant figures need not be shown.


The radius of a fluoride ion is larger than the radius of a fluorine atom.

The radius of F� is 73 pm greater than the radius of an F atom.

The F atom is 60 pm, the F� is 133 pm.

The F atom is smaller.


A lithium atom loses its second-shell electron, so the lithium ion has only one shell of electrons.

A lithium ion has one fewer electron.

The Li atom has 3 electrons and the Li� ion has 2 electrons.

A Li� ion has one less electron.

62 [1] Allow 1 credit. The positions of the dots may vary.

Examples of 1-credit responses:

��

��

��

�



As the elements in Period 2 are considered from left to right, the atomic radius generallydecreases.

The atomic radius goes down except for Neon.

The atomic radius gets smaller.


In this reaction, uranium is changing to other elements.

Different elements are formed.

One element becomes two new elements.

Two atoms are formed with different atomic numbers from the U-235.


9741Nb

97Nb

Nb−97

niobium−97


Part C

Allow a total of 20 credits for this part. The student must answer all questions in this part.


Fe oxidizes in the presence of Cu2� ions.

Iron is a more active metal than copper.

Cu2 ions act as an oxidizing agent.

Fe is above Cu on Table J.


5 � 10�4 mol

0.0005 mol


2H�(aq) � 2e�→ H2(g)

2H� � 2e�→ H2

2e� � 2H�1→ H2


Increase the concentration of the HCl(aq).

Increase the temperature.


Solute: NaClSolvent: H2O

Solute: sodium chlorideSolvent: water




The solution in beaker 4 has a greater ability to conduct an electric current because it has agreater concentration of aqueous ions than the solution in beaker 1.

There are fewer charged particles free to move in beaker 1.

There are more ions in beaker 4.


The greater the concentration of ions, the higher the boiling point of the solution.

The boiling point is lower with fewer dissolved particles.

The boiling point goes up with more aqueous ions.


From 0 to �2

From 0 to 2�

From zero to two


The number of moles of electrons lost is equal to the number of moles of electrons gained.

The number of moles is the same.

e� lost � e� gained.


Risk: Mercury is toxic.Benefit: Mercury batteries are miniature.

Risk: harmful to humansBenefit: producing electricity

35 04100 00 35 04 100

35135 100

35

.. .

gg g

g

��

�

((100)g g35 100�

77 [1] Allow 1 credit for yellow.

78 [1] Allow 1 credit for OH� or hydroxide.

79 [1] Allow 1 credit for 2 or two.

80 [1] Allow 1 credit for 0.86 M or 0.862 M.

81 [1] Allow 1 credit for carbon or C.


fermentation

fermenting


There is a double carbon-carbon bond in an ethene molecule.

Molecules of the compound contain a multiple C to C bond.

More H atoms can be added to the molecule.

Each molecule has C � C.


The alcohol functional group, �OH, allows for hydrogen bonding between ethanol molecules,so ethanol has a higher boiling point than ethene.

The boiling point of ethene is lower because its intermolecular forces are weaker than the intermolecular forces in the alcohol.

IMF for ethanol is stronger.


85 [1] Allow 1 credit.

Examples of 1-credit responses:

�

�

� �

�

�

�

��

�



The Chart for Determining the Final Examination Score for the August 2016Regents Examination in Physical Setting/Chemistry will be posted on the Department’s web site at: http://www.p12.nysed.gov/assessment/ onWednesday, August 17, 2016. Conversion charts provided for previous administrations of the Regents Examination in Physical Setting/Chemistrymust NOT be used to determine students’ final scores for this administration.

Regents Examination in Physical Setting/Chemistry

August 2016

Chart for Converting Total Test Raw Scores toFinal Examination Scores (Scale Scores)

Online Submission of Teacher Evaluations of the Test to the Department

Suggestions and feedback from teachers provide an important contribution to the test development process. The Department provides an online evaluation form for State assessments. It contains spaces for teachers to respond to several specific questions and tomake suggestions. Instructions for completing the evaluation form are as follows:

1. Go to http://www.forms2.nysed.gov/emsc/osa/exameval/reexameval.cfm.

2. Select the test title.

3. Complete the required demographic fields.

4. Complete each evaluation question and provide comments in the space provided.

5. Click the SUBMIT button at the bottom of the page to submit the completed form.


Map to Core Curriculum

August 2016 Physical Setting/Chemistry Question Numbers

Key Ideas/Performance Indicators Part A Part B Part C

Standard 1

Math Key Idea 1 41, 59 71, 79

Math Key Idea 2 40, 50, 51, 55, 65 73

Math Key Idea 3 32, 38, 41, 52, 59 67, 74, 80

Science Inquiry Key Idea 1

34, 36, 47, 51, 53,

54, 56, 57, 58, 60,

61, 63, 64

66, 69, 70, 72, 73,

75, 78, 77, 81, 82,

83, 84



33, 34, 35, 37, 42,

43, 46, 47, 48, 49, 54, 58, 60, 64, 65

66, 74, 77

Engineering Design Key Idea 1

Standard 2

Key Idea 1 31

Key Idea 2

Key Idea 3

Standard 6

Key Idea 1

Key Idea 2 46 68

Key Idea 3

32

Key Idea 4

Key Idea 5 51, 52, 55

Standard 7

Key Idea 1 76

Key Idea 2

Standard 4 Process Skills

Key Idea 3 39, 42, 44, 45, 51,

56, 63

67, 68, 71, 77, 80,

82, 85

Key Idea 4 33, 35, 37, 41, 54, 65

Key idea 5 34, 36, 62 84

Standard 4

Key Idea 3 1, 2, 3, 4, 5, 6, 10,

12, 13, 14, 15, 16,

17, 19, 20, 21, 23, 24, 25, 26, 27, 28,

30

31, 32, 33, 35, 39,

40, 42, 43, 44, 45,

46, 47, 48, 49, 50, 51, 52, 53, 55, 56,

57, 58, 63

66, 67, 68, 69, 70,

71, 72, 73, 74, 75,

76, 77, 78, 79, 80, 81, 82, 83, 85

Key Idea 4 18, 22, 29 41, 54, 59, 65

Key Idea 5 7, 8, 9, 11 34, 36, 37, 38, 60,

61, 62, 64

84

Reference Tables

2011 Edition 2, 3, 6, 7, 9, 10, 12,

15, 17, 26, 29

31, 33, 36, 38, 40,

41, 43, 45, 47, 50, 52, 57, 59, 61, 62,

63, 65

66, 68, 71, 74, 77,

78, 80, 81, 83, 85

P.S./Chemistry Conversion Chart - Aug. '16 1 of 1

Raw Scale Raw Scale Raw Scale Raw ScaleScore Score Score Score Score Score Score Score

85 100 62 74 39 57 16 3384 98 61 73 38 56 15 3183 97 60 72 37 56 14 2982 95 59 71 36 55 13 2881 94 58 71 35 54 12 2680 92 57 70 34 53 11 2479 91 56 69 33 52 10 2278 90 55 68 32 51 9 2077 88 54 68 31 50 8 1876 87 53 67 30 49 7 1675 86 52 66 29 49 6 1474 85 51 66 28 48 5 1273 84 50 65 27 46 4 1072 83 49 64 26 45 3 871 82 48 64 25 44 2 570 81 47 63 24 43 1 369 80 46 62 23 42 0 068 79 45 61 22 4167 78 44 61 21 4066 77 43 60 20 3865 76 42 59 19 3764 75 41 59 18 3563 74 40 58 17 34

Schools are not permitted to rescore any of the open-ended questions on this exam after each question hasbeen rated once, regardless of the final exam score. Schools are required to ensure that the raw scores havebeen added correctly and that the resulting scale score has been determined accurately.

Because scale scores corresponding to raw scores in the conversion chart change from one administration toanother, it is crucial that for each administration the conversion chart provided for that administration be used todetermine the student’s final score. The chart above is usable only for this administration of the Regents Examinationin Physical Setting/Chemistry.

The State Education Department / The University of the State of New York

Regents Examination in Physical Setting/Chemistry – August 2016Chart for Converting Total Test Raw Scores to Final Examination Scores (Scale Scores)

To determine the student’s final examination score, find the student’s total test raw score in the column labeled “RawScore” and then locate the scale score that corresponds to that raw score. The scale score is the student’s finalexamination score. Enter this score in the space labeled “Scale Score” on the student’s answer sheet.

Documents

PHYSICAL SETTING CHEMISTRY - JMAP · 2017-01-01 · Part A Answer all questions in this part. Directions (1–30): For each statement or question, record on your separate answer sheet